Question

For the Aufbau notation of Nd (Neodymium)

1. What is the last energy level and sublevel?
2. How many orbitals are drawn in that last sublevel?
3. How many electrons are paired up in that last sublevel?
4. How many electrons are single in that last sublevel?
5. How many empty orbitals are there in that last sublevel?

Answer 1

The last energy level and sublevel filled in Neodymium (Nd) is the 4f sublevel with 7 orbitals. All 14 electrons in the 4f sublevel are paired up, leaving no single electrons and no empty orbitals in the last sublevel.

Step-by-step explanation:

Aufbau Notation for Neodymium (Nd)

The Aufbau principle dictates that electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels. For the element Neodymium (Nd), with an atomic number of 60, the electron configuration will follow this rule.

1. The last energy level filled in Neodymium is the 4f sublevel.
2. There are 7 orbitals in the 4f sublevel.
3. All electrons in the 4f sublevel of Nd are paired up, which totals 14 electrons (since each orbital can hold 2 electrons).
4. There are no single electrons in the last sublevel of Neodymium as all orbitals are filled with paired electrons.
5. As all orbitals in the 4f sublevel are filled, there are no empty orbitals in this last sublevel for Nd.

To put it in electron configuration form, the notation for Nd would be [Xe] 6s²4f⁴, reflecting that the last electrons enter the 4f sublevel.